In the International System of Units ( \(SI\) ), the coulomb (\(C\)) is the preferred unit of electric charge quantity. It is equivalent to one ampere-second (\(1\,A.s\)) and represents approximately \(6.24 \times 10^{18}\) electric charge carriers. To convert from coulombs to faradays, multiply by \(1.04 \times 10^{-5}\).
ELECTROCHEMISTRY
19898
On passing \(0.1\) Faraday of electricity through aluminium chloride, the amount of aluminium metal deposited on cathode is \((Al = 27)\) ............ \(\mathrm{gm}\)
19899
Which of the following represents the first law of Faraday
1 \(E = m{c^2}\)
2 \(E = hv\)
3 \(m = ect\)
4 \(PV = nRT\)
Explanation:
The mass of the substance \(( m )\) deposited or liberated at any electrode is directly proportional to the quantity of electricity or charge (\(Q\)) passed.
ELECTROCHEMISTRY
19900
\(5\) amperes is passed through a solution of zinc sulphate for \(40 \) minutes. Find the amount of zinc deposited at the cathode ............. \(\mathrm{gm}\)
19901
In an electroplating experiment \(mg\) of silver is deposited, when \(4 \) amperes of current flows for \(2 \) minutes. The amount (in \(gms\)) of silver deposited by \( 6\) amperes of current flowing for \(40\) seconds will be
In the International System of Units ( \(SI\) ), the coulomb (\(C\)) is the preferred unit of electric charge quantity. It is equivalent to one ampere-second (\(1\,A.s\)) and represents approximately \(6.24 \times 10^{18}\) electric charge carriers. To convert from coulombs to faradays, multiply by \(1.04 \times 10^{-5}\).
ELECTROCHEMISTRY
19898
On passing \(0.1\) Faraday of electricity through aluminium chloride, the amount of aluminium metal deposited on cathode is \((Al = 27)\) ............ \(\mathrm{gm}\)
19899
Which of the following represents the first law of Faraday
1 \(E = m{c^2}\)
2 \(E = hv\)
3 \(m = ect\)
4 \(PV = nRT\)
Explanation:
The mass of the substance \(( m )\) deposited or liberated at any electrode is directly proportional to the quantity of electricity or charge (\(Q\)) passed.
ELECTROCHEMISTRY
19900
\(5\) amperes is passed through a solution of zinc sulphate for \(40 \) minutes. Find the amount of zinc deposited at the cathode ............. \(\mathrm{gm}\)
19901
In an electroplating experiment \(mg\) of silver is deposited, when \(4 \) amperes of current flows for \(2 \) minutes. The amount (in \(gms\)) of silver deposited by \( 6\) amperes of current flowing for \(40\) seconds will be
In the International System of Units ( \(SI\) ), the coulomb (\(C\)) is the preferred unit of electric charge quantity. It is equivalent to one ampere-second (\(1\,A.s\)) and represents approximately \(6.24 \times 10^{18}\) electric charge carriers. To convert from coulombs to faradays, multiply by \(1.04 \times 10^{-5}\).
ELECTROCHEMISTRY
19898
On passing \(0.1\) Faraday of electricity through aluminium chloride, the amount of aluminium metal deposited on cathode is \((Al = 27)\) ............ \(\mathrm{gm}\)
19899
Which of the following represents the first law of Faraday
1 \(E = m{c^2}\)
2 \(E = hv\)
3 \(m = ect\)
4 \(PV = nRT\)
Explanation:
The mass of the substance \(( m )\) deposited or liberated at any electrode is directly proportional to the quantity of electricity or charge (\(Q\)) passed.
ELECTROCHEMISTRY
19900
\(5\) amperes is passed through a solution of zinc sulphate for \(40 \) minutes. Find the amount of zinc deposited at the cathode ............. \(\mathrm{gm}\)
19901
In an electroplating experiment \(mg\) of silver is deposited, when \(4 \) amperes of current flows for \(2 \) minutes. The amount (in \(gms\)) of silver deposited by \( 6\) amperes of current flowing for \(40\) seconds will be
In the International System of Units ( \(SI\) ), the coulomb (\(C\)) is the preferred unit of electric charge quantity. It is equivalent to one ampere-second (\(1\,A.s\)) and represents approximately \(6.24 \times 10^{18}\) electric charge carriers. To convert from coulombs to faradays, multiply by \(1.04 \times 10^{-5}\).
ELECTROCHEMISTRY
19898
On passing \(0.1\) Faraday of electricity through aluminium chloride, the amount of aluminium metal deposited on cathode is \((Al = 27)\) ............ \(\mathrm{gm}\)
19899
Which of the following represents the first law of Faraday
1 \(E = m{c^2}\)
2 \(E = hv\)
3 \(m = ect\)
4 \(PV = nRT\)
Explanation:
The mass of the substance \(( m )\) deposited or liberated at any electrode is directly proportional to the quantity of electricity or charge (\(Q\)) passed.
ELECTROCHEMISTRY
19900
\(5\) amperes is passed through a solution of zinc sulphate for \(40 \) minutes. Find the amount of zinc deposited at the cathode ............. \(\mathrm{gm}\)
19901
In an electroplating experiment \(mg\) of silver is deposited, when \(4 \) amperes of current flows for \(2 \) minutes. The amount (in \(gms\)) of silver deposited by \( 6\) amperes of current flowing for \(40\) seconds will be
In the International System of Units ( \(SI\) ), the coulomb (\(C\)) is the preferred unit of electric charge quantity. It is equivalent to one ampere-second (\(1\,A.s\)) and represents approximately \(6.24 \times 10^{18}\) electric charge carriers. To convert from coulombs to faradays, multiply by \(1.04 \times 10^{-5}\).
ELECTROCHEMISTRY
19898
On passing \(0.1\) Faraday of electricity through aluminium chloride, the amount of aluminium metal deposited on cathode is \((Al = 27)\) ............ \(\mathrm{gm}\)
19899
Which of the following represents the first law of Faraday
1 \(E = m{c^2}\)
2 \(E = hv\)
3 \(m = ect\)
4 \(PV = nRT\)
Explanation:
The mass of the substance \(( m )\) deposited or liberated at any electrode is directly proportional to the quantity of electricity or charge (\(Q\)) passed.
ELECTROCHEMISTRY
19900
\(5\) amperes is passed through a solution of zinc sulphate for \(40 \) minutes. Find the amount of zinc deposited at the cathode ............. \(\mathrm{gm}\)
19901
In an electroplating experiment \(mg\) of silver is deposited, when \(4 \) amperes of current flows for \(2 \) minutes. The amount (in \(gms\)) of silver deposited by \( 6\) amperes of current flowing for \(40\) seconds will be
